The following data were obtained during the first thermal decomposition of `SO_2Cl_2` at a constant volume, `SO_2Cl_2(g) to SO_2 (g)+Cl_2 (g)` Experiment Time/s Total pressure/ atm 1 0 0.5 2 100 0.6 Calculate the rate of the reaction when total pressure is 0.65 atm.

The following data were obtained during the first order thermal decomposition of N_(2)O_(5)(g) at constant volume: 2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g) {:("SI.No","Time(s)","Pressure (atm)"),(1.,0,0.5),(2.,100,0.512):} Calculate the rate constant.

Following data were obtained during first order thermal decomposition of - SO_(2)Cl_(2)(g)rarrSO_(2)(g)+Cl_(2)(g) {:("Experiment","time"(s^(-1)),"Total pressure"("atm")),(1,0,0.4),(2,100,0.7):} Calculate the rate constant . (Given : log4 = 0.6021, log2 = 0.3010)

The following data were obtained during the first order thermal decomposition of N_(2)O_(5)(g) at constant volume. 2N_(2)O_(5)(g) rarr4NO_(2)(g)+O_(2)(g) {:(Time ("in s"),0,52,103,205,309),("Total pressure (in mm)",117.04,163.40,197.6,239.4,258.4):} Calculate the rate constant of the reaction.

Calculate the partial pressure of SO_2 in a mixture with 60% CO_2 and total pressure being 4 atm.

In the reaction, H_2(g) + Cl_2(g) iff 2HCl(g)

The value of K_p for the reaction 2H_2O(g) +2Cl_2(g) iff 4HCl(g) +O_2(g), is 0.035 atm at 400^@C , when the partial pressure are expressed in atmosphere. Calculate the value of K_c for the same reaction.

The equilibrium constant (K_P) for the decomposition of gaseous H_2O, H_2O(g)toH_2(g)+1/2O_2(g) , is related to degree of dissociation (prop) at a total pressure ( P) as-

The decomposition of gaseous Cl_(2)O_(7) to gaseous Cl_(2) and O_(2) at 400K is a first order reaction . After 55 s , the pressure of Cl_(2)O_(7) falls from 0.062 to 0.044 atm . Calculate the rate constant